Ionization energy decreases down the group and increases from left to right in a periodic table.
Ionization energy is defined as the amount of energy needed to remove a valance shell electron from an atom. In periodic table, Ionization energy decreases as we go from top to bottom in a group due to addition of more shells which make the outermost electron far away from the nucleus while on the other hand, Ionization energy increases when we move from left to right across the periodic table.
This is due to increase in number of protons in the nucleus which lowers the atomic radius so it is difficult to remove outermost electron of an atom or needs very high amount of energy so we can conclude that ionization energy decreases down the group and increases from left to right in a periodic table.
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